1.4 AS 90933 Demonstrate understanding of aspects of selected elements (4 credits)
Atomic structure and the organisation of the periodic table
− electron arrangement (limited to the first 20 elements)
− trend down a group (similarity of reaction, reactivity)
− trend across a period (position of metals and non-metals).
NCEA PAST EXAM QUESTIONS on Atomic structure
(a) Draw the electron arrangement for the atoms magnesium and chlorine
(b) Draw the electron arrangement for the magnesium and chloride ions
(c) Explain how magnesium and chlorine atoms react to form ions using the electron arrangements you have drawn above. Relate your answers to the positions of the atoms on the periodic table of elements.
Calcium, chlorine, fluorine and magnesium are all elements of the periodic table.
(a) Using the periodic table in your resource booklet, state the electron arrangements for the atoms fluorine and chlorine.
(b) Predict the number of valence electrons for bromine and iodine, and give an explanation for your choice.
(c) Explain how the formation of the calcium ion differs from the formation of the chloride ion, and relate this to the location of the elements on the periodic table.
(a) Write the electron arrangement for each of the elements magnesium, aluminium and sulphur.
(i) For the elements Magnesium and Sulfur, state whether each is a metal or a non-metal.
(ii) Explain how the elements magnesium and sulfur react to form the compound magnesium sulfide.
(a) (i) Using the Periodic Table in the Resource Booklet, give the electron arrangements of sodium and nitrogen.
(ii) Using these electron arrangements, explain how sodium and nitrogen differ in their ability to form ions.
(b) Compare and contrast the electron arrangements of the Group 1 metals, sodium and lithium.
Properties of metals (K, Na, Li, Mg, Ca, Al, Cu, Fe, Zn, Pb, Ag,) their reactivity and uses:
− activity series
− alloys.
Physical properties may include – melting and boiling points (state), colour, lustre, hardness, ductility and malleability, electrical and thermal conductivity, density.
Chemical properties may include reaction with oxygen, water and acids (HCl, H2SO4).
NCEA PAST EXAM QUESTIONS on uses of metals
Aluminium is widely used to make soft drink cans.
(i) Evaluate the use of aluminium for this purpose. Refer to BOTH physical and chemical properties of aluminium, and explain why they make aluminium suitable for making soft drink cans.
(ii) Name ONE metal that would be unsuitable as a material for making soft drink cans.
Justify your choice by referring to either a physical or a chemical property of the named metal.
You may refer to the activity series in the Resource Booklet.
Although copper is widely used throughout households for electrical wiring, aluminium is the metal used for long-distance power lines. Evaluate the advantages and disadvantages of using copper and aluminium in these roles.
Refer to BOTH physical and chemical properties in your answer.
Aluminium is used for packaging food and drink. Two such uses are aluminium foil and soft drink cans. Discuss the use of aluminium for packaging food and drink. In your answer, you should
state THREE physical properties of aluminium that make it suitable for making foil and soft drink can
explain why these physical properties make aluminium suitable for making foil and soft drink cans
fully explain why aluminium can be used in packaging food and drink even though it is chemically reactive.
Metals are good conductors of heat. Discuss how metals conduct heat and how this property can be applied in real life situations. Your answer should include:
how metals conduct heat (a diagram may be useful)
ONE example of how any of the metals copper, aluminium or iron are used in a way that depends on their thermal conductivity.
A craftsperson uses silver metal rather than iron metal to make body jewellery. Justify why the metal silver is more suitable for body jewellery than the metal iron. Include in your answer:
the relevant physical and chemical properties of silver metal
the relevant physical and chemical properties of iron metal
a justification as to why silver is preferable to iron for body jewellery.
One of the most common uses of aluminium is packaging, including soft drink cans and aluminium foil. Discuss why aluminium is used to package food and drinks despite the fact that aluminium is a reactive metal, found quite high up on the activity series (shown in your Resource Booklet). Include in your answer:
TWO or more properties that make aluminium suitable for making cans and foil
why aluminium can be used in packaging food and drink when the metal is quite reactive.
Sodium is not a metal that is usually used to make everyday objects, whereas aluminium is. For example, aluminium is used to make many objects from aeroplanes to soft drink cans. Discuss reasons for the difference in the uses of sodium and aluminium. Refer to the chemical and physical properties of both sodium and aluminium in your answer.
You have been asked to design a long-lasting metal roofing system for a house. The metals that are available are copper and iron. Discuss the suitability of each metal for a roofing system. Refer to relevant physical and chemical properties of each metal in your answer.
Gold is a metal that is often used to make jewellery. Name two properties of gold that make it suitable for this use. Explain why the two properties you named in part (a) help make gold suitable for making jewellery.
State the physical or chemical properties of aluminium that make the metal suitable for each of the uses given in the table below. Write a DIFFERENT PROPERTY in each cell of the table. Each property must relate to the given use.
Aluminium alloys are used to make planes and helicopters. Explain the advantages of using an aluminium alloy, rather than pure aluminium, for this purpose. In your answer, you will need to explain how the structure and properties of an alloy differ from those of a pure metal. You may use a labelled diagram to illustrate your answer.
Body piercing jewellery can be made from an alloy called ‘surgical steel’. Surgical steel is made from steel (iron and carbon) with nickel, molybdenum and chromium.
Each of the metals used to make surgical steel, shown in the table below, contributes to its final properties.
Evaluate why each of the metals listed in the table above is used to make surgical steel alloy suitable for use as body piercing jewellery. In your answer link ONE physical and ONE chemical property of each of these metals to its final use as body piercing jewellery.
1. Sterling silver is an alloy made of 92.5% silver and 7.5% copper.
(i) Describe ONE physical and ONE chemical property of pure silver that make it useful in the production of jewellery and other precious objects. You may refer to the activity series provided in the resource booklet.
(ii) Analyse the advantages and disadvantages of using sterling silver instead of pure silver in the production of jewellery and other precious objects. In your answer you should include physical and chemical properties of each of the metals used to make sterling silver. You may refer to the activity series provided in the resource booklet.
2. Developing alloys is an important industry worldwide. (a) Define the term alloy.
(b) Explain why an alloy is harder than a metal.In your answer refer to the diagrams below.
Alloys often have properties that are different from the properties of the metals they contain. This makes alloys more useful than pure metals alone. For example, an alloy may be harder than the metals from which it is made.(a) Explain why an alloy may be harder than the metals from which it is made. You may draw a labelled diagram in the box provided to support your answer. The table below gives some information about TWO alloys of gold.
(b) Discuss the use of different alloys of gold by jewellers. In your answer, you should
explain why both alloys described above are more useful to jewellers than pure gold
justify why a jeweller may prefer to use 18K gold to make a wedding ring but 9K gold to make a delicate necklace.
NCEA PAST EXAM QUESTIONS on Reactivity of metals with acids
Magnesium and copper are both metals used in the school laboratory. Elaborate on the reactivity of these two
metals in hydrochloric acid, HCl.
In your answer you should:
• identify any observations you would make when each of magnesium and copper are added separately to
hydrochloric acid
• link each observation to the reactants and products involved in the reaction
• write a balanced symbol equation for any reaction that occurs.
You may refer to the activity series in the Resource Booklet.
Small pieces of zinc were dropped into a test tube of dilute sulfuric acid solution.
(a) Describe the observations you would make of this reaction.
(b) Compare and contrast the reaction of zinc in dilute sulfuric acid solution with the reaction of iron in dilute sulfuric acid solution.
In your answer include the relevant balanced symbol equations.
You may refer to the activity series in the resource booklet.
Write both the observations and balanced equations for the reactions of sulfuric acid, H2SO4, with a cleaned piece of lead metal and with a cleaned piece of zinc metal.
You may refer to the Activity series in the Resource Booklet.
An investigation was carried out where identically sized pieces of the metals magnesium, zinc, and copper were placed in separate test tubes. The same volume and concentration of hydrochloric acid was added to each test tube.
(a) Describe the observations made during this investigation.
Magnesium and hydrochloric acid
Zinc and hydrochloric acid
Copper and hydrochloric acid
(b) Discuss the reactions that may occur with reference to the reactivity of the three metals. Include the balanced equations, where appropriate.
Refer to the activity series provided in the Resource Booklet.
Properties and uses of non-metals and selected compounds
− sulfur, aqueous chlorine, allotropes of carbon and oxygen (ozone), nitrogen, bromine and iodine
− selected compounds include – sulfuric acid, ammonia, sulfur dioxide.
Physical properties may include – melting and boiling points (state), colour, lustre, hardness, ductility and malleability, electrical and thermal conductivity, density.
Chemical properties may include reaction with oxygen.
NCEA PAST EXAM QUESTIONS on sulfur, sulfur dioxide and sulfuric acid
Sulfuric acid is used in lead-acid batteries that are used in cars.
The overall equation for the reactions that occur when the lead-acid car battery is being discharged (used) is:
Pb + PbO2+ 2H2SO4→ 2PbSO4+ 2H2O
Lead sulfate, PbSO4, forms as the battery discharges.
Analyse the role of the sulfuric acid solution in the reactions of the lead-acid battery.
In your answer include:
• the properties of sulfuric acid solution that make it a good conductor of electricity
• how the concentration of sulfuric acid changes while the battery is discharging AND while it is charging.
1. Sulfur in its pure form reacts with oxygen.
(a) Describe an observation made of the product formed in the reaction of sulfur with oxygen.
(b) Write a balanced equation for this reaction
2. Pure water is a poor conductor of electricity, but a solution of sulfuric acid in water is a good electrical conductor.
Explain why the sulfuric acid solution conducts electricity so well. Include a balanced equation in your answer
A solution of sulfuric acid in water is used in lead-acid batteries found in cars
Discuss the role of sulfuric acid solution in the reactions of a lead-acid battery.
Your answer should include:
• the properties of sulfuric acid that make it a good electrolyte
• how sulfuric acid is involved in the reactions that occur when the battery is discharging and when it is charging
• how the concentration of sulfuric acid changes while the battery is discharging and while it is charging
(a) Chlorine water is formed by adding chlorine gas to water. Some of the chlorine dissolves in water and some reacts with water. Explain what happens to a piece of blue litmus paper when it is used to test the chlorine water. In your answer you should:
• describe the observations you would make of the blue litmus paper
• explain your observations by linking them to the properties of the chlorine water
• write a balanced symbol equation for the reaction of chlorine gas with water
(b) In hospitals, chlorine-based solutions are used in cleaning and disinfecting to help protect patients from infection. Justify why chlorine-based solutions are used in hospitals by explaining how the chemical properties of chlorine-based solutions make them suitable for cleaning and disinfecting.
Chlorine may be added to water in swimming pools to make the water safe for people. Discuss the chemistry involved in using chlorine to treat swimming pool water. In your answer, you should:
write a word equation for the reaction of chlorine with water
explain how chlorine forms an acidic solution when it reacts with water
write a balanced chemical equation for the reaction of chlorine with water
fully explain how a particular product of the reaction of chlorine with water makes the water safe for people to swim.
Chlorine is the chemical most often used to keep swimming pools and spa pools free from bacteria. Too many bacteria can be hazardous to human health.
Discuss the properties and reactions of chlorine that enable it to keep pool water clean.
(a) Explain how chlorine reacts with water.
Include a relevant balanced equation.
(b) Explain how the addition of chlorine keeps the pool water free from bacteria.
(c) Explain why chlorine needs to be added to pool water at regular intervals.
Atomic structure and the organisation of the periodic table
− electron arrangement (limited to the first 20 elements)
− trend down a group (similarity of reaction, reactivity)
− trend across a period (position of metals and non-metals).
NCEA PAST EXAM QUESTIONS on Atomic structure
(a) Draw the electron arrangement for the atoms magnesium and chlorine
(b) Draw the electron arrangement for the magnesium and chloride ions
(c) Explain how magnesium and chlorine atoms react to form ions using the electron arrangements you have drawn above. Relate your answers to the positions of the atoms on the periodic table of elements.
Calcium, chlorine, fluorine and magnesium are all elements of the periodic table.
(a) Using the periodic table in your resource booklet, state the electron arrangements for the atoms fluorine and chlorine.
(b) Predict the number of valence electrons for bromine and iodine, and give an explanation for your choice.
(c) Explain how the formation of the calcium ion differs from the formation of the chloride ion, and relate this to the location of the elements on the periodic table.
(a) Write the electron arrangement for each of the elements magnesium, aluminium and sulphur.
(i) For the elements Magnesium and Sulfur, state whether each is a metal or a non-metal.
(ii) Explain how the elements magnesium and sulfur react to form the compound magnesium sulfide.
(a) (i) Using the Periodic Table in the Resource Booklet, give the electron arrangements of sodium and nitrogen.
(ii) Using these electron arrangements, explain how sodium and nitrogen differ in their ability to form ions.
(b) Compare and contrast the electron arrangements of the Group 1 metals, sodium and lithium.
Properties of metals (K, Na, Li, Mg, Ca, Al, Cu, Fe, Zn, Pb, Ag,) their reactivity and uses:
− activity series
− alloys.
Physical properties may include – melting and boiling points (state), colour, lustre, hardness, ductility and malleability, electrical and thermal conductivity, density.
Chemical properties may include reaction with oxygen, water and acids (HCl, H2SO4).
NCEA PAST EXAM QUESTIONS on uses of metals
Aluminium is widely used to make soft drink cans.
(i) Evaluate the use of aluminium for this purpose. Refer to BOTH physical and chemical properties of aluminium, and explain why they make aluminium suitable for making soft drink cans.
(ii) Name ONE metal that would be unsuitable as a material for making soft drink cans.
Justify your choice by referring to either a physical or a chemical property of the named metal.
You may refer to the activity series in the Resource Booklet.
Although copper is widely used throughout households for electrical wiring, aluminium is the metal used for long-distance power lines. Evaluate the advantages and disadvantages of using copper and aluminium in these roles.
Refer to BOTH physical and chemical properties in your answer.
Aluminium is used for packaging food and drink. Two such uses are aluminium foil and soft drink cans. Discuss the use of aluminium for packaging food and drink. In your answer, you should
state THREE physical properties of aluminium that make it suitable for making foil and soft drink can
explain why these physical properties make aluminium suitable for making foil and soft drink cans
fully explain why aluminium can be used in packaging food and drink even though it is chemically reactive.
Metals are good conductors of heat. Discuss how metals conduct heat and how this property can be applied in real life situations. Your answer should include:
how metals conduct heat (a diagram may be useful)
ONE example of how any of the metals copper, aluminium or iron are used in a way that depends on their thermal conductivity.
A craftsperson uses silver metal rather than iron metal to make body jewellery. Justify why the metal silver is more suitable for body jewellery than the metal iron. Include in your answer:
the relevant physical and chemical properties of silver metal
the relevant physical and chemical properties of iron metal
a justification as to why silver is preferable to iron for body jewellery.
One of the most common uses of aluminium is packaging, including soft drink cans and aluminium foil. Discuss why aluminium is used to package food and drinks despite the fact that aluminium is a reactive metal, found quite high up on the activity series (shown in your Resource Booklet). Include in your answer:
TWO or more properties that make aluminium suitable for making cans and foil
why aluminium can be used in packaging food and drink when the metal is quite reactive.
Sodium is not a metal that is usually used to make everyday objects, whereas aluminium is. For example, aluminium is used to make many objects from aeroplanes to soft drink cans. Discuss reasons for the difference in the uses of sodium and aluminium. Refer to the chemical and physical properties of both sodium and aluminium in your answer.
You have been asked to design a long-lasting metal roofing system for a house. The metals that are available are copper and iron. Discuss the suitability of each metal for a roofing system. Refer to relevant physical and chemical properties of each metal in your answer.
Gold is a metal that is often used to make jewellery. Name two properties of gold that make it suitable for this use. Explain why the two properties you named in part (a) help make gold suitable for making jewellery.
State the physical or chemical properties of aluminium that make the metal suitable for each of the uses given in the table below. Write a DIFFERENT PROPERTY in each cell of the table. Each property must relate to the given use.
NCEA PAST EXAM QUESTIONS on Alloys
Aluminium alloys are used to make planes and helicopters. Explain the advantages of using an aluminium alloy, rather than pure aluminium, for this purpose. In your answer, you will need to explain how the structure and properties of an alloy differ from those of a pure metal. You may use a labelled diagram to illustrate your answer.
Body piercing jewellery can be made from an alloy called ‘surgical steel’. Surgical steel is made from steel (iron and carbon) with nickel, molybdenum and chromium.
Each of the metals used to make surgical steel, shown in the table below, contributes to its final properties.
Evaluate why each of the metals listed in the table above is used to make surgical steel alloy suitable for use as body piercing jewellery. In your answer link ONE physical and ONE chemical property of each of these metals to its final use as body piercing jewellery.
1. Sterling silver is an alloy made of 92.5% silver and 7.5% copper.
(i) Describe ONE physical and ONE chemical property of pure silver that make it useful in the production of jewellery and other precious objects. You may refer to the activity series provided in the resource booklet.
(ii) Analyse the advantages and disadvantages of using sterling silver instead of pure silver in the production of jewellery and other precious objects. In your answer you should include physical and chemical properties of each of the metals used to make sterling silver. You may refer to the activity series provided in the resource booklet.
2. Developing alloys is an important industry worldwide. (a) Define the term alloy.
(b) Explain why an alloy is harder than a metal.In your answer refer to the diagrams below.
Alloys often have properties that are different from the properties of the metals they contain. This makes alloys more useful than pure metals alone. For example, an alloy may be harder than the metals from which it is made.(a) Explain why an alloy may be harder than the metals from which it is made. You may draw a labelled diagram in the box provided to support your answer. The table below gives some information about TWO alloys of gold.
(b) Discuss the use of different alloys of gold by jewellers. In your answer, you should
explain why both alloys described above are more useful to jewellers than pure gold
justify why a jeweller may prefer to use 18K gold to make a wedding ring but 9K gold to make a delicate necklace.
NCEA PAST EXAM QUESTIONS on Reactivity of metals with oxygen
Compare and contrast the reaction of magnesium and oxygen with the reaction of sulfur (non-metal) and
oxygen. In your answer you should:
• identify any observations you would make for each reaction
• link each observation to the chemical species involved in each reaction
• write a balanced symbol equation for each reaction.
The metals calcium and copper may react when heated in oxygen.
The table below gives the observations made when calcium and copper are heated in oxygen
Discuss the reactivities of calcium and copper metals. In your answer, you should:
identify the chemical products formed in any reactions
link the chemical products formed to the observations given in the table
write balanced equations for the reactions that occur
fully explain why calcium is placed before copper on the Activity Series (refer to the resource booklet).
NCEA PAST EXAM QUESTIONS on Reactivity of metals with water
Calcium and magnesium are Group 2 metals. Analyse the reactions these metals have with cold water.
In your answer include:
• observations you would make for both metals reacting with water
• any links these observations would have to the products formed in each reaction
• an explanation of any similarities and differences in the reactivity of these two metals in water
• a balanced symbol equation for ONE of these reactions.
Lithium and sodium are both Group 1 metals. Analyse the type of reaction that these metals have with water. In your answer include:
• observations of lithium and sodium reacting with water
• a word and balanced symbol equation of ONE of these reactions
• a comparison of the reactivity of lithium and sodium, with water.
The metals calcium and copper may react when put into water.
The table below gives the observations made when calcium and copper are put into water.
Discuss the reactivities of calcium and copper metals. In your answer, you should:
identify the chemical products formed in any reactions
link the chemical products formed to the observations given in the table
write balanced equations for the reactions that occur
fully explain why calcium is placed before copper on the Activity Series (refer to the resource booklet).
NCEA PAST EXAM QUESTIONS on Reactivity of metals with acids
Magnesium and copper are both metals used in the school laboratory. Elaborate on the reactivity of these two
metals in hydrochloric acid, HCl.
In your answer you should:
• identify any observations you would make when each of magnesium and copper are added separately to
hydrochloric acid
• link each observation to the reactants and products involved in the reaction
• write a balanced symbol equation for any reaction that occurs.
You may refer to the activity series in the Resource Booklet.
Small pieces of zinc were dropped into a test tube of dilute sulfuric acid solution.
(a) Describe the observations you would make of this reaction.
(b) Compare and contrast the reaction of zinc in dilute sulfuric acid solution with the reaction of iron in dilute sulfuric acid solution.
In your answer include the relevant balanced symbol equations.
You may refer to the activity series in the resource booklet.
Write both the observations and balanced equations for the reactions of sulfuric acid, H2SO4, with a cleaned piece of lead metal and with a cleaned piece of zinc metal.
You may refer to the Activity series in the Resource Booklet.
An investigation was carried out where identically sized pieces of the metals magnesium, zinc, and copper were placed in separate test tubes. The same volume and concentration of hydrochloric acid was added to each test tube.
(a) Describe the observations made during this investigation.
Magnesium and hydrochloric acid
Zinc and hydrochloric acid
Copper and hydrochloric acid
(b) Discuss the reactions that may occur with reference to the reactivity of the three metals. Include the balanced equations, where appropriate.
Refer to the activity series provided in the Resource Booklet.
Properties and uses of non-metals and selected compounds
− sulfur, aqueous chlorine, allotropes of carbon and oxygen (ozone), nitrogen, bromine and iodine
− selected compounds include – sulfuric acid, ammonia, sulfur dioxide.
Physical properties may include – melting and boiling points (state), colour, lustre, hardness, ductility and malleability, electrical and thermal conductivity, density.
Chemical properties may include reaction with oxygen.
NCEA PAST EXAM QUESTIONS on sulfur, sulfur dioxide and sulfuric acid
Sulfuric acid is used in lead-acid batteries that are used in cars.
The overall equation for the reactions that occur when the lead-acid car battery is being discharged (used) is:
Pb + PbO2+ 2H2SO4→ 2PbSO4+ 2H2O
Lead sulfate, PbSO4, forms as the battery discharges.
Analyse the role of the sulfuric acid solution in the reactions of the lead-acid battery.
In your answer include:
• the properties of sulfuric acid solution that make it a good conductor of electricity
• how the concentration of sulfuric acid changes while the battery is discharging AND while it is charging.
1. Sulfur in its pure form reacts with oxygen.
(a) Describe an observation made of the product formed in the reaction of sulfur with oxygen.
(b) Write a balanced equation for this reaction
2. Pure water is a poor conductor of electricity, but a solution of sulfuric acid in water is a good electrical conductor.
Explain why the sulfuric acid solution conducts electricity so well. Include a balanced equation in your answer
A solution of sulfuric acid in water is used in lead-acid batteries found in cars
Discuss the role of sulfuric acid solution in the reactions of a lead-acid battery.
Your answer should include:
• the properties of sulfuric acid that make it a good electrolyte
• how sulfuric acid is involved in the reactions that occur when the battery is discharging and when it is charging
• how the concentration of sulfuric acid changes while the battery is discharging and while it is charging
• any relevant balanced equations.
NCEA PAST EXAM QUESTIONS on aqueous chlorine
(a) Chlorine water is formed by adding chlorine gas to water. Some of the chlorine dissolves in water and some reacts with water. Explain what happens to a piece of blue litmus paper when it is used to test the chlorine water. In your answer you should:
• describe the observations you would make of the blue litmus paper
• explain your observations by linking them to the properties of the chlorine water
• write a balanced symbol equation for the reaction of chlorine gas with water
(b) In hospitals, chlorine-based solutions are used in cleaning and disinfecting to help protect patients from infection. Justify why chlorine-based solutions are used in hospitals by explaining how the chemical properties of chlorine-based solutions make them suitable for cleaning and disinfecting.
Chlorine may be added to water in swimming pools to make the water safe for people. Discuss the chemistry involved in using chlorine to treat swimming pool water. In your answer, you should:
write a word equation for the reaction of chlorine with water
explain how chlorine forms an acidic solution when it reacts with water
write a balanced chemical equation for the reaction of chlorine with water
fully explain how a particular product of the reaction of chlorine with water makes the water safe for people to swim.
Chlorine is the chemical most often used to keep swimming pools and spa pools free from bacteria. Too many bacteria can be hazardous to human health.
Discuss the properties and reactions of chlorine that enable it to keep pool water clean.
(a) Explain how chlorine reacts with water.
Include a relevant balanced equation.
(b) Explain how the addition of chlorine keeps the pool water free from bacteria.
(c) Explain why chlorine needs to be added to pool water at regular intervals.
Download this FREE live preview of an EXCEPTIONALLY student friendly Level 1 Chemistry workbook
SciPAD (2015) Jason Rendle, Silverback Academic Media